Name: strong acids, strong bases, and ph
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 22 s
Channel: JoVE

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Strong Acid and Base Solutions

الأحماض القوية تتفك كليًا في الماء. على سبيل المثال،حمض النيتريك يتفكك بالكامل إلى أيونات هيدرونيوم وأيونات نترات. بما أن أيونات الهيدرونيوم،الناشئة عن تأين الماء التلقائي،ضئيلة جدًا،يكون تركيز أيونات الهيدرونيوم في الماء مساويًا لتركيز الحمض القوي.يمكن تحديد قيمة pH لهذه المحاليل باستخدام التركيز الأولي للحمض القوي. على سبيل المثال،في محلول HCl ذو تركيز 0.10 مولار،سيتفكك HCl بالكامل إلى أيونات هيدرونيوم وأيونات كلوريد،وبالتالي سيكون تركيز الهيدرونيوم في المحلول 0.10 مولار. بأخذ اللوغاريتمات السالبة لهذا التركيز فإن قيمة pH لهذا المحلول تساوي واحد.وعلى العكس،يمكن استخدام قيمة pH لمحلول،لتحديد تركيز أيونات الهيدرونيوم في المحلول. على سبيل المثال،محلول فيه pH يساوي 3.60،يمكن تحديد تركيز أيونات الهيدرونيوم فيه بحل المعادلة بحيث 3.60 تساوي اللوغاريتم السالب لتركيز أيونات الهيدرونيوم. لإيجاد قيمة التركيز،نضرب الطرفين في سالب واحد،ثم نأخذ مضاد اللوغاريثم للطرفين.تركيز أيونات الهيدرونيوم يساوي 2.5 10⁻⁴ مولار. القواعد القوية،وهي هيدروكسيدات فلزية مثل هيدروكسيد الصوديوم،وهيدروكسيد البوتاسيوم،تتفك بالكامل في المحلول. على سبيل المثال،0.20 مولار من هيدروكسيد الصوديوم ستتفكك كليًا في الماء وتنتج 0.20 مولار من أيونات الصوديوم،و0.20 مولار من أيونات الهيدروكسيد.غير أن الهيدروكسيدات الفلزية من الفئة الثانية،مثل هيدروكسيد الباريوم،وهيدروكسيد الكالسيوم،تنتج 2 مول من أيونات الهيدروكسيد مقابل كل مول من القاعدة. على سبيل المثال،0.020 مولار من هيدروكسيد الكالسيوم ستتفكك كليًا في الماء وستنتج 0.020 مولار من أيونات الكالسيوم،و0.040 مولار من أيونات الهيدروكسيد. الأكسيدات الفلزية الأيونية،كأكسيد الصوديوم وأكسيد الكالسيوم،هي الأخرى قواعد قوية.تتفاعل أيوناتها الأكسيدية مع الماء وتنتج أيونات هيدروكسيد. تركيز أيونات الهيدروكسيد،يمكن استخدامه لحساب قيمة pOH و pH للمحلول. على سبيل المثال،محلول هيدروكسيد البوتاس الذي تركيز أيوناته 5 10⁻⁵ مول،يحتوي كمية مساوية من أيونات الهيدروكسيد،باعتباره قاعدة قوية وبالتالي تكون قيمة pOH فيه 4.30.قيمة pOH في المحلول،يمكن استخدامها مثل قيمة pH لتحديد تركيز أيونات الهيدروكسيد بحل المعادلة:pOH تساوي اللوغاريتم السالب لتركيز أيونات الهيدروكسيد. بما أن pH زائد pOH تساوي 14 وبما أن pOH يساوي 4.3،تكون قيمة pH للمحلول 9.7.

حمض قوي ومحاليل أساسية

الحمض القوي مركب ينفصل تمامًا في محلول مائي وينتج تركيز أيونات الهيدرونيوم يساوي التركيز الأولي للحمض. على سبيل المثال ، سينفصل حمض الهيدروبروميك 0.20 مولار تمامًا في الماء وتنتج 0.20 م من أيونات الهيدرونيوم و 0.20 م من أيونات البروميد. <img alt = "" Eq1 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_1.png "" style = "" height: 50px؛ "" / > من ناحية أخرى ، القاعدة القوية عبارة عن مركب ينفصل تمامًا في محلول مائي وينتج أيونات الهيدروكسيد. على سبيل المثال ، 0.015 M KOH، وهي مجموعة هيدروكسيد فلز من المجموعة 1 ، سوف تنفصل تمامًا وتنتج 0.015 M من OH - و 0.015 M من K + . <img alt = "" Eq2 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_2.png "" style = "" height: 50px؛ "" / > هيدروكسيدات المعادن من المجموعة 2 ، مثل هيدروكسيد الباريوم [Ba (OH) 2 ] وهيدروكسيد السترونشيوم [Sr (OH) 2 ] ، هي أيضًا قواعد قوية وتمتلك اثنين أيونات الهيدروكسيد. هذا يجعلهم ينتجون محلولًا أكثر أساسية مقارنة بـ NaOH أو KOH بنفس التركيز. على سبيل المثال ،Ba(OH)2  ينتج 0.015 M Ba+  and 0.030 M hydroxide. <img alt = "" Eq3 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_3.png "" style = "" height: 50px؛ "" / > نظرًا لانفصال الأحماض والقواعد القوية تمامًا ، يمكن استخدام النسب المولية لتحديد تركيزات الهيدرونيوم والهيدروكسيد ، والتي يمكن استخدامها بدورها لحساب الأس الهيدروجيني أو الأس الهيدروجيني لمحلول ما. على سبيل المثال ، سينتج محلول حمض الهيدروكلوريك 0.030 مولار 0.03 مولار من أيونات الهيدرونيوم. لذلك سيكون الرقم الهيدروجيني لهذا المحلول <img alt = "" Eq4 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_4.png "" style = "" height: 135px؛ "" / > يمكن تحديد الرقم الهيدروجيني لنفس المحلول باستخدام الصيغة <img alt = "" Eq5 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_5.png "" style = "" height: 50px؛ "" / > نظرًا لأن الرقم الهيدروجيني للمحلول هو 1.52 ، يمكن حساب الأس الهيدروجيني الخاص به على أنه <img alt = "" Eq6 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_6.png "" style = "" height: 50px؛ "" / > وبالمثل ، يمكن استخدام تركيز أيونات الهيدروكسيد الناتجة عن قواعد قوية لتحديد الأس الهيدروجيني لمحلول باستخدام المعادلة <img alt = "" Eq7 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_7.png "" style = "" height: 50px؛ "" / > يمكن أيضًا استخدام المعادلة أعلاه لتحديد تركيز أيون الهيدروكسيد عندما يكون الهيدروكسيد معروفًا. على سبيل المثال ، إذا كان الرقم الهيدروجيني للحل هو 3.00 ، <img alt = "" Eq8 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_8.png "" style = "" height: 50px؛ "" / > ضرب كلا الجانبين بـ & # 8722 ؛ 1 يعطي <img alt = "" Eq9 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_9.png "" style = "" height: 50px؛ "" / > الآن ، خذ مضاد كلا الجانبين <img alt = "" Eq10 "" src = "" / files / ftp_upload / 11399 / 11399_Equation_10.png "" style = "" height: 90px؛ "" / > وبالتالي ، فإن تركيز أيون الهيدرونيوم للمحلول مع pOH 3 هو 1.0 & # 215 ؛ 10 & # 8722؛ 3 M. يمكن استخدام طريقة مماثلة لتحديد تركيز أيون الهيدرونيوم لمحلول إذا كان الرقم الهيدروجيني معروفًا.

الحمض القوي هو مركب يتفكك تماما في محلول مائي وينتج تركيزا من أيونات الهيدرونيوم يساوي ...

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Acids and Bases

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strong acids, strong bases, and ph

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio.

For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates completely. It produces 0.015 M OH- and 0.015 M K+.

Some group 2 metal hydroxides are also strong bases. Barium hydroxide, Ba(OH)2, and strontium hydroxide, Sr(OH)2, each contain two hydroxide ions. That means they create a more basic solution than NaOH or KOH at the same concentration. For example, 0.015 M Ba(OH)2 produces 0.015 M Ba+ and 0.030 M hydroxide.

The ion concentrations from strong acids and strong bases can be used to calculate pH and pOH. A 0.030 M HCl solution produces 0.03 M hydronium ions, so its pH can be found from that concentration. The same pH value can then be used to determine pOH. If the pH is 1.52, the pOH can be calculated from the relationship between them.

The same idea works for strong bases. The hydroxide ion concentration can be used to find pOH with the equation for pOH, and the equation can also be used in reverse when pOH is known. For example, if the pOH of a solution is 3.00, multiplying by -1 and taking the antilog gives a hydronium ion concentration of 1.0 × 10^-3 M. The same method can be used to find hydronium ion concentration when pH is known.

Strong Acids, Strong Bases, and pH

bronsted-lowry acids and bases

Proton Transfer in Acids and Bases

Acids and bases can be understood through proton transfer. Early scientists described acids by their sour taste, their effect on dyes, and their reaction with limestone, which releases carbon dioxide. Robert Boyle also noted that acid solutions can lose these properties after contact with alkali, or base, solutions. The modern view developed step by step. Humphry Davy showed that hydrogen is the essential part of acids. Joseph Louis Gay-Lussac then described acids as substances that neutralize...

water: a bronsted-lowry acid and base

Water as an Amphiprotic Substance

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

ph scale

pH and pOH in Water

pH and pOH show how hydronium and hydroxide ions behave in water and other aqueous solutions. These ion concentrations are linked by the ion product of water, K w , so when one goes up, the other goes down. Because ion concentrations can differ by huge amounts, a logarithmic scale is used to describe them. pH is defined from the hydronium ion concentration, [H3O+], and pOH is the matching p-function for hydroxide ion concentration. These two values are also connected through the K w...

relative strengths of conjugate acid-base pairs

relative-strengths-of-conjugate-acid-base-pairs

How Ka and Kb Show Acid-Base Strength

Brønsted-Lowry acid-base chemistry is based on proton transfer. That idea helps show how the strength of an acid is linked to the strength of its conjugate base, and vice versa. Acid and base strength is measured with ionization constants, Ka and Kb, which tell how far an ionization reaction goes. For the conjugate pair HA and A−, the acid ionizes in water and the base reaction can be written for the partner species. When the two reactions are added, they give the autoionization of water. The...

strong acid and base solutions

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio. For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates...

weak acid solutions

Weak Acid Equilibrium in Water

Weak acid equilibrium in water explains why many acids only partially react when dissolved. Most weak acid molecules stay in their original form, and only a small amount of hydronium ions forms. Weak acids are common in nature. They help create the tangy taste of citrus fruits, the stinging sensation from insect bites, and the smells linked to body odor. Acetic acid is a familiar weak acid. It is the main ingredient in vinegar. Its equation uses a double arrow to show that the reaction with...

weak base solutions

Weak Base pH and Kb Calculations

Weak base pH and Kb calculations show how partially reacting bases change water chemistry. Weak bases produce hydroxide ions when they dissolve by reacting with water molecules. Because the reaction only happens partly, these compounds are classified as weak bases. Weak bases are common in nature and in technology. Ammonia is one major example. Global production of ammonia is typically well over 100 metric tons each year. It is used as an agricultural fertilizer, a starting material for...

mixtures of acids

pH of Acid Mixtures

The pH of acid mixtures depends on the acids present, their dissociation constants, and their starting concentrations. When a solution contains two different acids, the pH can be found by choosing the method that fits their relative strengths. This makes acid mixtures a useful case for applying acid-base rules in chemistry. In a mixture of a strong acid and a weak acid, the strong acid dissociates completely and supplies almost all of the hydronium ions in the solution. The weak acid...

ions as acids and bases

Salt Hydrolysis and pH of Solutions

Salt hydrolysis explains why some salt solutions are acidic, basic, or neutral. Salts are ionic compounds made of cations and anions. In water, either ion may react with water through an acid or base ionization reaction. The pH of the solution depends on the relative acid-base strength of the ions in the salt. Ammonium chloride is a good example of an acidic salt. When it dissolves, it separates into ammonium ions and chloride ions. The ammonium ion is the conjugate acid of ammonia, so it can...

determining the ph of salt solutions

Salt Hydrolysis and pH in Solutions

Salt hydrolysis and pH in solutions depend on the ions released when a salt dissolves. Some ions react with water, while others do not. The balance between the cation and anion helps show whether the solution becomes acidic, basic, or neutral. Salts with pH-neutral anions and cations that produce hydronium ions give acidic solutions with pH below 7. Ammonium nitrate is one example. In NH4NO3, NO3− does not react with water, but NH4+ forms hydronium ions, so the solution is acidic. Other salts...

acid/base strengths and dissociation constants

acidbase-strengths-and-dissociation-constants

Acid and Base Strength in Water

Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones. The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water. <br...

polyprotic acids

Stepwise Ionization of Polyprotic Acids

Polyprotic acids lose hydrogen ions in steps. The number of ionizable protons in a molecule determines whether an acid is monoprotic, diprotic, or triprotic. This video also shows that polyprotic bases can accept more than one proton. Monoprotic acids have one ionizable hydrogen atom per molecule. Examples include HCl, HNO3, and HCN. Their reactions with water form hydronium ions and the matching anion. Acetic acid, CH3CO2H, is also monoprotic because only the hydrogen in the carboxyl group...

acid strength and molecular structure

How Bonding Affects Acid Strength

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases. For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as...

lewis acids and bases

Electron-Pair Reactions in Acid-Base Chemistry

Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

key terms and concepts

Learn how strong acids and strong bases dissociate completely in water and how their ion concentrations are used to calculate pH and pOH.

Strong Acids, Strong Bases, and pH | JoVE K12

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Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

PS.Chm.3.2

Analyze the structure of atoms and isotopes.

Strong Acids, Strong Bases, and pH

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